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Hydrometallurgy of Lead

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Hydrometallurgy of Lead NEW TECHNOLOGY FOR LEAD Fathi Habashi Department of Mining, Metallurgical, and Materials Engineering Laval University, Quebec City, Canada e-mail: [email protected] Lead is an ancient metal, has been produced to-date from its ores exclusively by pyrometallurgical route. The process suffers from numerous steps, high operating cost, and excessive pollution problems. Galena PbS Metallurgy of lead Refining of lead Refining of lead • The complex refining steps and the pollution in the neighborhood of smelters are causing much trouble to the nearby population • For example, the high content of lead in crab collected from the ocean in the vicinity of a lead smelter worries consumers • The appreciable amounts of lead in wine produced from a vineyard near a lead smelter causes concern to the industry. • The maximum permissible limit for lead in the vicinity of a smelter is 0.05 mg Pb/m3 of air or 6 ppb, a limit that is difficult to achieve in many plants. • In addition, lead smelters produce SO2 and this must be converted to sulfuric acid. • A nearby market for the acid must exist. otherwise SO2 will have to be emitted in the environment, which is unacceptable. • As a result, a number of smelters and refineries have been shut down. • Both problems can only be solved by using a hydrometallurgical route to process the sulfide concentrate. • No lead fumes will be emitted in the environment and elemental sulfur could be produced, which is easy to store or ship to sulfuric acid manufacturers. Hydrometallurgy of lead • Extensive research has been going on since the beginning of the twentieth century to find a non- polluting process for its production and a solution for its complex refining scheme. • It has been assumed correctly that the hydrometallurgical route should be the most promising. • Pilot plants have been constructed and operated for a reasonable periods, but no process has proved to be fully satisfactory until recently. First hydrometallurgical attempts • O. C. Ralston US Bureau of Mines in Berkeley, California 1924 The solubility of PbCl2 and PbSO4 in brine solutions Tainton at Bunker Hill in Kellogg, Idaho 1924 PbS concentrate O2 Roasting SO2 H2O PbSO4, impurities Leaching Filtration Impurities CaCl2 Leaching Filtration Gangue, CaSO4 2- PbCl4 Cl2 Absorption Aq. Electrolysis Ca(OH)2 Refining Ag Pb Failure of Tainton Process • Although it was supposed to be a sulfation roasting, yet some SO2 was formed. • In the electrowinning step chlorine was formed and was not disposed of properly beside its corrosion problems. • Lead powder obtained was not satisfactorily handled and was contaminated by silver. Bunker Hill Process in Kellogg, Idaho (1960s). High temperature aqueous oxidation (220oC) PbS Concentrate O2 H2O Aq. Oxidation Filtration CuSO4, ZnSO4 PbSO4, Ag2SO4 Blast Furnace CO2, SO2 Crude Pb Refining Ag Pb Problems with Bunker Hill Process • The process was thought to be more advantageous than the roasting process because no SO2 would be evolved. • In fact it was not, since SO2 was generated in the blast furnace gases due to the decomposition of lead sulfate. Other processes Galena is attacked by dilute acids generating H2S: + 2+ PbS + 2H → Pb + H2S which can be collected and converted by standard technology to elemental sulfur at 400ºC using alumina as catalyst: H2S + ½ O2 → S + H2O However, the toxicity of H2S and its explosive nature renders this route undesirable Galena is attacked by concentrated H2SO4 at 100ºC to form SO2 and elemental sulfur: PbS + 2H2SO4 → PbSO4 + SO2 + S + 2H2O The reaction is simple but offers no special advantage since SO2 is generated. Aqueous oxidation of PbS in acid Aqueous oxidation of PbS in acid results in the formation of elemental sulfur: + 2+ PbS + ½ O2 + 2H → Pb + S + H2O • When H2SO4 is used, PbSO4 will be formed and when HCl is used then PbCl2 will be formed together with an appreciable amount of PbSO4 since a portion 2- of sulfide sulfur is oxidized to SO4 and other components of the concentrate will form soluble sulfates. • Solution purification can be achieved by cementation of the impurities with lead powder. Ferrous ion can then be oxidized back to ferric for recycle. Oxidation may take place by oxygen: 2+ + 3+ Fe + ½O2 + 2H → 2Fe + H2O • Or by chlorine when FeCl3 is used: 2+ 3+ - 2Fe + Cl2(aq) → 2Fe + 2Cl There is no advantage in using the sulfate system because of the difficulties encountered in the recovery step. When Fe3+ ion is used instead of oxygen the following reaction takes place: PbS + 2Fe3+ → Pb2+ + 2Fe2+ + S Processing lead sulfide concentrates with formation of elemental sulfur. Chloride system PbS concentrate Fe3+ HCl Aq. Oxidation Filtration Soluble chlorides Flotation S Brine Leaching Filtration Gangue Fe 2+ oxidation Crystallization PbCl2 Cl2 Electolysis Pb US Bureau of Mines Process in Reno, Nevada • In this case chlorine could be obtained from the electrolysis of PbCl2 either in aqueous solution (complexed with NaCl) or in the molten state. • This was the basis of the processes developed by researchers at US Bureau of Mines and others. • This shows again that the chloride system is more preferable than the sulfate system, since in the latter case the sulfate ion must be disposed of. • Oxidation of Fe2+ may also be achieved in the electrolytic step whereby the evolution of chlorine is suppressed as proposed by French researchers. Carbonate system To avoid the formation of PbSO4 or PbCl2, aqueous oxidation of PbS was conducted by Chinese researchers in presence of ammonium carbonate at about 50°C. Lead carbonate and elemental sulfur are formed: PbS + (NH4)2CO3 + ½O2 + H2O → PbCO3 + S + 2NH4OH • Residence time about 6 hours and yield of sulfur is 60%. After flotation of elemental sulfur, PbCO3 was solubilized in fluorosilicic acid, the solution purified, then electrolyzed for electrowinning of lead. PbS concentrate (NH4)2CO3 O2 Aq. Oxidation Filtration Recovery Solids Flotation S, Ag H2SiF6 PbCO3, gangue Dissolution Filtration Residue containing Ag Purification Impurities Electrolysis Pb NITRATE SYSTEM • The nitrate system has the advantage that both lead and silver will go into solution and hence separation can be readily achieved. • Using HNO3, however, has the disadvantage of generating nitric gases, which must be re- converted to HNO3. • The use of ferric nitrate was already proposed. the following reaction takes place: PbS + 2Fe(NO3)3 → Pb(NO3)2 + 2Fe(NO3)2 + S • Complete dissolution of galena took place at 70°C in 0.25 M Fe(NO3)3 solution at pH 1.2- 1.4 in 100 minutes. • While lead forms at the cathode, PbO2 forms at the anode. PbS concentrate Fe(NO3)3 Leaching Filtration Flotation Solution Heating Gangue S NO + NO2 Regeneration Filtration HNO3 Fe 2O3 Solution Dissolution Purification Bi, Cu, Ag, Zn Electrolysis Pb + PbO2 – After purification of the solution from copper and bismuth by cementation on lead and the separation, if necessary, of zinc by organic solvents, lead can be recovered by electrowinning at the cathode as Pb and at the anode as PbO2: - - Pb(NO3)2 + 2e Pb + 2NO3 - - Pb(NO3)2 + 2H2O + 2NO3 PbO2 + 4HNO3 + 2e Overall reaction 2Pb(NO3)2 + 2H2O Pb + PbO2 + 4HNO3 CHLORINATION The use of gaseous chlorine has the advantage over the aqueous chloride system is the absence of PbSO4 formation since all the sulfide sulfur is transformed to the elemental form. There have been early attempts in this direction at the beginning of the twentieth century but without success owing to the difficulties encountered in handling chlorine. About sixty years later, researchers at the US Bureau of Mines in Rolla, Missouri re-examined this technology and recommended the recovery of lead by the electrolysis of fused PbCl2. A pilot plant was later operated at Hazen Research Center in Golden, Colorado based on such technology. Chlorine gas is fed to rotating reactor counter-current to the flow of fresh concentrate so that any sulfur monochloride formed becomes the chlorinating agent: PbS + Cl2 PbCl2 + S 2S + Cl2 S2Cl2 PbS + S2Cl2 PbCl2 + 3S The temperature in the reactor is155-175C. • Lead chloride and other chlorinated compounds are then solubilized in hot brine solution. Lead chloride is then crystallized and, the anhydrous PbCl2 is fed in a fused salt cell containing 90% PbCl2 and 10% NaCl and operating at 500C. • High purity lead was obtained. • Mother liquor from crystallization step is treated with sponge iron to remove silver. A bleed stream is treated with NaOH or Na2CO3 to remove other impurities. • Work at Universal Oil Products laboratory in Des Plaines, Illinois also confirmed this technology. FLUOROSILICATE SYSTEM • Since lead fluorosilicate is soluble in water, it was suggested by workers at US Bureau of Mines in Rolla, Missouri to leach lead sulfide concentrate in fluorosilicic acid: • PbS + H2SiF6 + ½O2 PbSiF6 + S + H2O • After filtration of the residue and solution purification, lead can be recovered by electrolysis. The residue contained elemental sulfur, silver, zinc, and copper. • Attempts to electrowin lead from the leach solution were not successful because of low current efficiency and undesirable cathode morphology due to impurities present. • To overcome this problem, the Bureau of Mines researchers suggested adding H2SO4 to precipitate PbSO4, transform the sulfate into carbonate, dissolving PbCO3 in H2SiF6, then electrolyzing the pure lead fluorosilicate solution. • High purity lead was obtained but the procedure suffers from the numerous steps involved and the generation of ammonium sulfate as a by-product. PbS concentrate
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